Introductory Chemistry: Concepts and Critical Thinking

Charles H. Corwin

Chapter 18

Oxidation and Reduction - all with Video Answers

Educators

Chapter Questions

Problem 1

Which class of hydrocarbon is saturated?

Sima Sarker

Sima Sarker

Numerade Educator

Problem 1

State the oxidation number for each of the following elements in the free state:
(a) Au
(b) Mn
(c) P
(d) $\mathrm{O}_{2}$

Sima Sarker

Numerade Educator

Problem 2

What is the primary source of hydrocarbons?

Zaida Minjares

Numerade Educator

Problem 2

State the oxidation number for each of the following elements in the free state:
(a) Ag
(b) $\mathrm{Mg}$
(c) S
(d) $F_{2}$

Sima Sarker

Numerade Educator

Problem 3

State the oxidation number for each of the following monoatomic ions:
(a) $\mathrm{Au}^{3+}$
(b) $\mathrm{Mn}^{2+}$
(c) $P^{3-}$
(d) $\mathrm{O}^{2-}$

Sima Sarker

Numerade Educator

Problem 3

Which classes of hydrocarbon are unsaturated?

Sima Sarker

Numerade Educator

Problem 4

State the oxidation number for each of the following monoatomic ions:
(a) $\mathrm{Ag}^{+}$
(b) $\mathrm{Mg}^{2+}$
(c) $S^{2-}$
(d) $\mathrm{F}^{-}$

Sima Sarker

Numerade Educator

Problem 4

Which class of hydrocarbon has only single bonds?

Sima Sarker

Numerade Educator

Problem 5

Calculate the oxidation number for nitrogen in the following compounds:
(a) $\mathrm{NH}_{3}$
(b) $\mathrm{N}_{2} \mathrm{O}_{4}$
(c) $\mathrm{Li}_{3} \mathrm{~N}$
(d) $\mathrm{KNO}_{3}$

Ivan Kochetkov

Numerade Educator

Problem 5

Which class of hydrocarbon has double bonds?

Sima Sarker

Numerade Educator

Problem 6

Calculate the oxidation number for silicon in the following compounds:
(a) $\mathrm{Si}_{2} \mathrm{H}_{6}$
(b) $\mathrm{SiO}_{2}$
(c) $\mathrm{Si}_{2} \mathrm{~N}_{4}$
(d) $\mathrm{CaSiO}_{3}$

Sima Sarker

Numerade Educator

Problem 6

Which class of hydrocarbon has triple bonds?

Sima Sarker

Numerade Educator

Problem 7

Which of the following molecular formulas represents an alkane?
(a) $\mathrm{C}_{10} \mathrm{H}_{24}$
(b) $C_{10} H_{22}$

Sima Sarker

Numerade Educator

Problem 7

Calculate the oxidation number for sulfur in the following polyatomic ions:
(a) $\mathrm{SO}_{3}^{2-}$
(b) $\mathrm{HSO}_{4}$
(c) HS
(d) $\mathrm{S}_{2} \mathrm{O}_{8}{ }^{2-}$

Sima Sarker

Numerade Educator

Problem 8

What is the molecular formula for each of the following alkanes?
(a) $\mathrm{C}_{11} \mathrm{H}_{2}$
(b) $\mathrm{C}_{12} \mathrm{H}_{2}$

Sima Sarker

Numerade Educator

Problem 8

Calculate the oxidation number for carbon in the following polyatomic ions:
(a) $\mathrm{CO}_{3}^{2-}$
(b) $\mathrm{HCO}_{3}^{-}$
(c) CN
(d) CNO

Sima Sarker

Numerade Educator

Problem 9

State the name for each of the following alkanes:
(a) $\mathrm{CH}_{3}-\mathrm{CH}_{2}-\mathrm{CH}_{3}$
(b) $\mathrm{CH}_{3}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{3}$
(c) $\mathrm{CH}_{3}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{3}$
(d) $\mathrm{CH}_{3}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{3}$

Sima Sarker

Numerade Educator

Problem 9

Supply the term that corresponds to each of the following:
(a) a redox process characterized by electron gain
(b) a substance causing reduction in a redox reaction

Ivan Kochetkov

Numerade Educator

Problem 10

Draw the condensed structural formula for each of the following alkanes:
(a) ethane
(b) butane
(c) hexane
(d) octane

Sima Sarker

Numerade Educator

Problem 10

Supply the term that corresponds to each of the following:
(a) a redox process characterized by electron loss
(b) a substance causing oxidation in a redox reaction

Ivan Kochetkov

Numerade Educator

Problem 11

State the substances undergoing oxidation and reduction in the following redox reactions:
(a) $\mathrm{Co}(s)+\mathrm{S}(s) \longrightarrow \operatorname{CoS}(s)$
(b) $\mathrm{Cd}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CdCl}_{2}(\mathrm{~s})$

Ivan Kochetkov

Numerade Educator

Problem 12

State the substances undergoing oxidation and reduction in the following redox reactions:
(a) $\mathrm{Mg}(s)+\mathrm{S}(s) \longrightarrow \mathrm{MgS}(s)$
(b) $\mathrm{Mn}(s)+\mathrm{Br}_{2}(l) \longrightarrow \operatorname{MnBr}_{2}(s)$

Ivan Kochetkov

Numerade Educator

Problem 13

Indicate the oxidizing and reducing agents in the following redox reactions:
(a) $\mathrm{CuO}(s)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{Cu}(s)+\mathrm{H}_{2} \mathrm{O}(l)$
(b) $\mathrm{PbO}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Pb}(s)+\mathrm{CO}_{2}(g)$

Ivan Kochetkov

Numerade Educator

Problem 14

Indicate the oxidizing and reducing agents in the following redox reactions:
(a) $\mathrm{Ca}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{2}(g)$
(b) $\mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g)$

Ivan Kochetkov

Numerade Educator

Problem 15

Indicate the substances undergoing oxidation and reduction in the following ionic redox reactions:
(a) $\mathrm{Al}(s)+\mathrm{Cr}^{3+}(a q) \longrightarrow \mathrm{Al}^{3+}(a q)+\mathrm{Cr}(s)$
(b) $\mathrm{F}_{2}(g)+2 \mathrm{Cl}^{-}(a q) \longrightarrow 2 \mathrm{~F}(a q)+\mathrm{Cl}_{2}(g)$

Ivan Kochetkov

Numerade Educator

Problem 16

Indicate the substances undergoing oxidation and reduction in the following ionic redox reactions:
(a) $\mathrm{Fe}^{3+}(a q)+\mathrm{SO}_{3}^{2-}(a q) \longrightarrow \mathrm{Fe}^{2+}(a q)+\mathrm{SO}_{4}^{2-}(a q)$
(b) $\mathrm{Cl}_{2}(g)+2 \mathrm{I}(a q) \longrightarrow 2 \mathrm{Cl}^{-}(a q)+\mathrm{I}_{2}(s)$

Ivan Kochetkov

Numerade Educator

Problem 17

Indicate the oxidizing and reducing agents in the following redox reactions:
(a) $\mathrm{Cr}^{2+}(a q)+\mathrm{AgI}(s) \longrightarrow \mathrm{Cr}^{3+}(a q)+\mathrm{Ag}(s)+\Gamma(a q)$
(b) $\operatorname{Sn}^{2+}(a q)+\mathrm{Hg}^{2+}(a q) \longrightarrow \mathrm{Sn}^{4+}(a q)+\mathrm{Hg}_{2}^{2+}(a q)$

Ivan Kochetkov

Numerade Educator

Problem 18

Indicate the oxidizing and reducing agents in the following redox reactions:
(a) $\mathrm{H}_{2} \mathrm{O}_{2}(a q)+\mathrm{SO}_{3}{ }^{2-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{SO}_{4}{ }^{2-}(a q)$
(b) $\mathrm{IO}_{3}^{-}(a q)+\mathrm{Cu}^{+}(a q) \longrightarrow \mathrm{Cu}^{2+}(a q)+\mathrm{I}_{2}(s)$

Ivan Kochetkov

Numerade Educator

Problem 19

Does the electron loss by oxidation always equal the electron gain by reduction in a balanced redox equation?

Sima Sarker

Numerade Educator

Problem 20

Does the total ionic charge on the reactants always equal the total ionic charge on the products in a balanced redox equation?

Sima Sarker

Numerade Educator

Problem 21

Write a balanced equation for each of the following redox reactions using the oxidation number method:
(a) $\mathrm{Br}_{2}(l)+\operatorname{NaI}(a q) \longrightarrow \mathrm{I}_{2}(s)+\operatorname{NaBr}(a q)$
(b) $\mathrm{PbS}(\mathrm{s})+\mathrm{O}_{2}(g) \longrightarrow \mathrm{PbO}(a q)+\mathrm{SO}_{2}(g)$

Ivan Kochetkov

Numerade Educator

Problem 22

Write a balanced equation for each of the following redox reactions using the oxidation number method:
(a) $\mathrm{Cl}_{2}(g)+\mathrm{KI}(a q) \longrightarrow \mathrm{I}_{2}(s)+\mathrm{KCl}(a q)$
(b) $\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g)$

Ivan Kochetkov

Numerade Educator

Problem 23

Write a balanced equation for each of the following redox reactions using the oxidation number method:
(a) $\mathrm{MnO}_{4}^{-}(a q)+\mathrm{I}^{-}(a q)+\mathrm{H}^{+}(a q) \longrightarrow$
$$
\mathrm{Mn}^{2+}(a q)+\mathrm{I}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l)
$$
(b) $\mathrm{Cu}(s)+\mathrm{H}^{+}(a q)+\mathrm{SO}_{4}^{2-}(a q) \longrightarrow$
$$
\mathrm{Cu}^{2+}(a q)+\mathrm{SO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)
$$

Ivan Kochetkov

Numerade Educator

Problem 24

Write a balanced equation for each of the following redox reactions using the oxidation number method:
$$
\begin{array}{l}
\text { (a) } \mathrm{Fe}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}_{2}(a q)+\mathrm{H}^{+}(a q) \longrightarrow \mathrm{Fe}^{3+}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \\
\text { (b) } \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{Br}^{-}(a q)+\mathrm{H}^{+}(a q) \longrightarrow \mathrm{Cr}^{3+}(a q)+\mathrm{Br}_{2}(l)+\mathrm{H}_{2} \mathrm{O}(l)
\end{array}
$$

Ivan Kochetkov

Numerade Educator

Problem 25

Write a balanced half-reaction for each of the following in an acidic solution:
(a) $\mathrm{SO}_{2}(g) \longrightarrow \mathrm{SO}_{4}{ }^{2-}(a q)$
(b) $\mathrm{BrO}_{3}^{-}(a q) \longrightarrow \mathrm{Br}_{2}(l)$

Ivan Kochetkov

Numerade Educator

Problem 26

Write a balanced half-reaction for each of the following in an acidic solution:
(a) $\mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)$
(b) $\mathrm{AsO}_{3}^{3-}(a q) \longrightarrow \mathrm{AsO}_{3}^{-}(a q)$

Ivan Kochetkov

Numerade Educator

Problem 27

Write a balanced half-reaction for each of the following in a basic solution:
(a) $\mathrm{ClO}^{-}(a q) \longrightarrow \mathrm{Cl}^{-}(a q)$
(b) $\mathrm{MnO}_{4}^{-}(a q) \longrightarrow \mathrm{MnO}_{2}(s)$

Ivan Kochetkov

Numerade Educator

Problem 28

Write a balanced half-reaction for each of the following in a basic solution:
(a) $\mathrm{Ni}(\mathrm{OH})_{2}(s) \longrightarrow \mathrm{NiO}_{2}(s)$
(b) $\mathrm{NO}_{2}^{-}(a q) \longrightarrow \mathrm{N}_{2} \mathrm{O}(g)$

Ivan Kochetkov

Numerade Educator

Problem 29

Write a balanced equation for each of the following redox reactions in an acidic solution using the half-reaction method:
(a) $\mathrm{Zn}(\mathrm{s})+\mathrm{NO}_{3}^{-}(a q) \longrightarrow \mathrm{Zn}^{2+}(a q)+\mathrm{NO}(g)$
(b) $\mathrm{Mn}^{2+}(a q)+\mathrm{BiO}_{3}^{-}(a q) \longrightarrow \mathrm{MnO}_{4}^{-}(a q)+\mathrm{Bi}^{3+}(a q)$

Ivan Kochetkov

Numerade Educator

Problem 30

Write a balanced equation for each of the following redox reactions in an acidic solution using the half-reaction method:
(a) $\mathrm{Sn}^{2+}(a q)+\mathrm{IO}_{3}^{-}(a q) \longrightarrow \mathrm{Sn}^{4+}(a q)+\mathrm{I}_{2}(s)$
(b) $\mathrm{AsO}_{3}^{3-}(a q)+\mathrm{Br}_{2}(l) \longrightarrow \mathrm{AsO}_{4}{ }^{3-}(a q)+\mathrm{Br}^{-}(a q)$

Ivan Kochetkov

Numerade Educator

Problem 31

Write a balanced equation for each of the following redox reactions in a basic solution using the half-reaction method:
(a) $\mathrm{MnO}_{4}^{-}(a q)+\mathrm{S}^{2-}(a q) \longrightarrow \mathrm{MnO}_{2}(s)+\mathrm{S}(s)$
(b) $\mathrm{Cu}(s)+\mathrm{ClO}^{-}(a q) \longrightarrow \mathrm{Cu}^{2+}(a q)+\mathrm{Cl}^{-}(a q)$

David Collins

Numerade Educator

Problem 32

Write a balanced equation for each of the following redox reactions in a basic solution using the half-reaction method:
(a) $\mathrm{Cl}_{2}(g)+\mathrm{BrO}_{2}^{-}(a q) \longrightarrow \mathrm{Cl}^{-}(a q)+\mathrm{BrO}_{3}^{-}(a q)$
(b) $\mathrm{MnO}_{2}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{MnO}_{4}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$

David Collins

Numerade Educator

Problem 33

Chlorine can undergo a redox reaction in which it is simultaneously oxidized and reduced. Write a balanced equation for the following in an acidic solution:
$$
\mathrm{Cl}_{2}(a q) \longrightarrow \mathrm{Cl}^{-}(a q)+\mathrm{HOCl}(a q)
$$

Ivan Kochetkov

Numerade Educator

Problem 34

Nitrous acid, $\mathrm{HNO}_{2}$, can undergo a redox reaction in which it is simultaneously oxidized and reduced. Write a balanced equation for the following in an acidic solution:
$$
\mathrm{HNO}_{2}(a q) \longrightarrow \mathrm{NO}_{3}^{-}(a q)+\mathrm{NO}(g)
$$

Ivan Kochetkov

Numerade Educator

Problem 35

Chlorine can undergo a redox reaction in which it is simultaneously oxidized and reduced. Write a balanced equation for the following in a basic solution:
$$
\mathrm{Cl}_{2}(a q) \longrightarrow \mathrm{ClO}_{2}^{-}(a q)+\mathrm{Cl}^{-}(a q)
$$

Ivan Kochetkov

Numerade Educator

Problem 36

Sulfur can undergo a redox reaction in which it is simultaneously oxidized and reduced. Write a balanced equation for the following in a basic solution:
$$
\mathrm{S}(s) \longrightarrow \mathrm{SO}_{3}^{2-}(a q)+\mathrm{S}^{2-}(a q)
$$

Ivan Kochetkov

Numerade Educator

Problem 37

Refer to Figure 4 and indicate which substance in each of the following pairs has the greater tendency to be oxidized:
(a) $\mathrm{Li}(s)$ or $\mathrm{K}(s)$
(b) $\mathrm{Al}(s)$ or $\mathrm{Mg}(s)$
(c) $\mathrm{Fe}^{2+}(a q)$ or $\mathrm{I}(a q)$
(d) $\mathrm{Br}^{-}(a q)$ or $\mathrm{Cl}^{-}(a q)$

Sima Sarker

Numerade Educator

Problem 38

Refer to Figure 4 and indicate which substance in each of the following pairs has the greater tendency to be reduced:
(a) $\mathrm{Pb}^{2+}(a q)$ or $\mathrm{Zn}^{2+}(a q)$
(b) $\mathrm{Fe}^{3+}(a q)$ or $\mathrm{Al}^{3+}(a q)$
(c) $\mathrm{Ag}^{+}(a q)$ or $\mathrm{I}_{2}(\mathrm{~s})$
(d) $\mathrm{Cu}^{2+}(a q)$ or $\mathrm{Br}_{2}(l)$

Sima Sarker

Numerade Educator

Problem 39

Refer to Figure 4 and indicate which substance in each of the following pairs is the stronger oxidizing agent:
(a) $\mathrm{F}_{2}(g)$ or $\mathrm{Cl}_{2}(g)$
(b) $\mathrm{Ag}^{+}(a q)$ or $\mathrm{Br}_{2}(l)$
(c) $\mathrm{Cu}^{2+}(a q)$ or $\mathrm{H}^{+}(a q)$
(d) $\mathrm{Mg}^{2+}(a q)$ or $\mathrm{Mn}^{2+}(a q)$

Sima Sarker

Numerade Educator

Problem 40

Refer to Figure 4 and indicate which substance in each of the following pairs is the stronger reducing agent:
(a) $\mathrm{Cu}(s)$ or $\mathrm{Cr}(s)$
(b) $\mathrm{H}_{2}(g)$ or $\mathrm{Cu}(s)$
(c) $\mathrm{Cu}(\mathrm{s})$ or $\mathrm{I}^{-}(a q)$
(d) $\mathrm{Cl}^{-}(a q)$ or $\mathrm{H}_{2}(g)$

Sima Sarker

Numerade Educator

Problem 41

Refer to Figure 4 and state whether each of the following reactions is spontaneous or nonspontaneous:
(a) $\mathrm{Br}_{2}(l)+\mathrm{LiF}(a q) \longrightarrow \mathrm{F}_{2}(s)+\mathrm{LiBr}(a q)$
(b) $\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{Mn}(s) \longrightarrow \mathrm{Mn}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Al}(s)$

Sima Sarker

Numerade Educator

Problem 42

Refer to Figure 4 and state whether each of the following reactions is spontaneous or nonspontaneous:
(a) $\mathrm{Cr}(\mathrm{s})+\mathrm{HCl}(a q) \longrightarrow \mathrm{CrCl}_{3}(a q)+\mathrm{H}_{2}(g)$
(b) $\mathrm{FeCl}_{3}(a q)+\operatorname{NaI}(a q) \longrightarrow \mathrm{FeCl}_{2}(a q)+\mathrm{NaCl}(a q)+\mathrm{I}_{2}(s)$

David Collins

Numerade Educator

Problem 43

Refer to Figure 4 and state whether each of the following ionic redox reactions is spontaneous or nonspontaneous:
(a) $\mathrm{Mg}(\mathrm{s})+\mathrm{Sn}^{2+}(a q) \stackrel{\text { ? }}{\longrightarrow} \mathrm{Mg}^{2+}(a q)+\mathrm{Sn}(\mathrm{s})$
(b) $\mathrm{H}^{+}(a q)+\mathrm{Ni}(s) \longrightarrow \mathrm{H}_{2}(g)+\mathrm{Ni}^{2+}(a q)$

Sima Sarker

Numerade Educator

Problem 44

Refer to Figure 4 and state whether each of the following ionic redox reactions is spontaneous or nonspontaneous:
(a) $\mathrm{H}^{+}(a q)+\mathrm{I}(a q) \longrightarrow \mathrm{H}_{2}(g)+\mathrm{I}_{2}(s)$
(b) $\mathrm{Fe}^{3+}(a q)+\mathrm{I}(a q) \longrightarrow \mathrm{Fe}^{2+}(a q)+\mathrm{I}_{2}(s)$

Sima Sarker

Numerade Educator

Problem 45

Given the following redox reactions, list $\mathrm{A}, \mathrm{B},$ and $\mathrm{C}$ according to which is higher in the table of reduction potentials:
$$
\begin{array}{l}
\mathrm{A}(s)+\mathrm{B}^{+}(a q) \longrightarrow \mathrm{B}(s)+\mathrm{A}^{+}(a q) \\
\mathrm{B}(s)+\mathrm{C}^{+}(a q) \longrightarrow \mathrm{C}(s)+\mathrm{B}^{+}(a q)
\end{array}
$$

Ivan Kochetkov

Numerade Educator

Problem 46

Given the following redox reactions, list $X, Y,$ and $Z$ according to which is higher in the table of reduction potentials:
$$
\begin{array}{l}
\mathrm{X}_{2}(a q)+2 \mathrm{Y}^{-}(a q) \longrightarrow \mathrm{Y}_{2}(a q)+2 \mathrm{X}^{-}(a q) \\
\mathrm{Y}_{2}(a q)+2 \mathrm{Z}^{-}(a q) \longrightarrow \mathrm{Z}_{2}(a q)+2 \mathrm{Y}^{-}(a q)
\end{array}
$$

David Collins

Numerade Educator

Problem 47

Sketch the following voltaic cell showing the two compartments, the anode and cathode, the wire connecting the two electrodes, and a salt bridge:
$$
\mathrm{Ni}(s)+2 \mathrm{AgNO}_{3}(a q) \longrightarrow 2 \mathrm{Ag}(s)+\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)
$$

David Collins

Numerade Educator

Problem 48

Sketch the following voltaic cell showing the two compartments, the anode and cathode, the wire connecting the two electrodes, and a salt bridge:
$$
\mathrm{Mn}(s)+\mathrm{Cd}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow \mathrm{Cd}(s)+\mathrm{Mn}\left(\mathrm{NO}_{3}\right)_{2}(a q)
$$

David Collins

Numerade Educator

Problem 49

Diagram the direction of electron flow and the movement of nitrate ions in the salt bridge that connects the two halfcells in Exercise 47

David Collins

Numerade Educator

Problem 50

Diagram the direction of electron flow and the movement of nitrate ions in the salt bridge that connects the two halfcells in Exercise $48 .$

David Collins

Numerade Educator

Problem 51

The spontaneous redox reaction of manganese and aqueous iron(II) sulfate occurs according to the following ionic equation:
$$
\mathrm{Mn}(s)+\mathrm{Fe}^{2+}(a q) \longrightarrow \mathrm{Mn}^{2+}(a q)+\mathrm{Fe}(a q)
$$
The half-reactions are separated into two compartments. A Mn electrode is placed in $1.00 \mathrm{M} \mathrm{MnSO}_{4},$ and an Fe electrode in $1.00 \mathrm{M} \mathrm{FeSO}_{4}$. Indicate each of the following for the voltaic cell.
(a) oxidation half-cell reaction
(b) reduction half-cell reaction
(c) anode and cathode
(d) direction of electron flow
(e) direction of $\mathrm{SO}_{4}{ }^{2-}$ in the salt bridge

Sima Sarker

Numerade Educator

Problem 52

The spontaneous redox reaction of tin and aqueous copper(II) sulfate occurs according to the following ionic equation:
$$
\mathrm{Sn}(s)+\mathrm{Cu}^{2+}(a q) \longrightarrow \mathrm{Cu}(s)+\mathrm{Sn}^{2+}(a q)
$$
The half-reactions are separated into two compartments. A Sn electrode is placed in $1.00 \mathrm{M} \mathrm{SnSO}_{4},$ and a Cu electrode in $1.00 \mathrm{M} \mathrm{CuSO}_{4}$. Indicate each of the following for the voltaic cell:
(a) oxidation half-cell reaction
(b) reduction half-cell reaction
(c) anode and cathode
(d) direction of electron flow
(e) direction of $\mathrm{SO}_{4}^{2-}$ in the salt bridge

Sima Sarker

Numerade Educator

Problem 53

The spontaneous redox reaction of magnesium and aqueous lead(II) nitrate occurs according to the following equation:
$$
\mathrm{Mg}(\mathrm{s})+\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow \mathrm{Pb}(\mathrm{s})+\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)
$$
The half-reactions are separated into two compartments. A Mg electrode is placed in $1.00 \mathrm{M} \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2},$ and a $\mathrm{Pb}$ electrode in $1.00 M \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2} .$ Indicate each of the following for the voltaic cell:
(a) oxidation half-cell reaction
(b) reduction half-cell reaction
(c) anode and cathode
(d) direction of electron flow
(e) direction of $\mathrm{NO}_{3}^{-}$ in the salt bridge

Sima Sarker

Numerade Educator

Problem 54

The spontaneous redox reaction of cobalt and aqueous manganese(II) nitrate occurs according to the following equation:
$$
\mathrm{Mn}(s)+\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow \mathrm{Co}(s)+\mathrm{Mn}\left(\mathrm{NO}_{3}\right)_{2}(a q)
$$
The half-reactions are separated into two compartments. A Mn electrode is placed in $1.00 \mathrm{M} \mathrm{Mn}\left(\mathrm{NO}_{3}\right)_{2},$ and a Co electrode in $1.00 \mathrm{M} \mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2} .$ Indicate each of the following for the voltaic cell:
(a) oxidation half-cell reaction
(b) reduction half-cell reaction
(c) anode and cathode
(d) direction of electron flow
(e) direction of $\mathrm{NO}_{3}^{-}$ in the salt bridge

Sima Sarker

Numerade Educator

Problem 55

The nonspontaneous redox reaction of nickel and aqueous iron(II) sulfate is an electrolytic process according to the following equation:
$$
\mathrm{Ni}(s)+\mathrm{FeSO}_{4}(a q) \longrightarrow \mathrm{Fe}(s)+\mathrm{NiSO}_{4}(a q)
$$
The half-reactions are separated into two compartments. A Ni electrode is placed in $1.00 \mathrm{M} \mathrm{NiSO}_{4}$, and an Fe electrode in $1.00 \mathrm{M} \mathrm{FeSO}_{4}$. Indicate each of the following for the electrolytic cell:
(a) oxidation half-cell reaction
(b) reduction half-cell reaction
(c) anode and cathode
(d) direction of electron flow
(e) direction of $\mathrm{SO}_{4}{ }^{2-}$ in the salt bridge

Sima Sarker

Numerade Educator

Problem 56

The nonspontaneous redox reaction of tin and aqueous cobalt(II) sulfate is an electrolytic process according to the following equation:
$$
\mathrm{Sn}(s)+\operatorname{CoSO}_{4}(a q) \longrightarrow \mathrm{Co}(s)+\mathrm{SnSO}_{4}(a q)
$$
The half-reactions are separated into two compartments. A Sn electrode is placed in $1.00 \mathrm{MSnSO}_{4}$, and a Co electrode in $1.00 \mathrm{M} \mathrm{CoSO}_{4}$. Indicate each of the following for the electrolytic cell:
(a) oxidation half-cell reaction
(b) reduction half-cell reaction
(c) anode and cathode
(d) direction of electron flow
(e) direction of $\mathrm{SO}_{4}{ }^{2-}$ in the salt bridge

David Collins

Numerade Educator

Problem 57

The nonspontaneous redox reaction of lead metal and aqueous zinc nitrate is an electrolytic process according to the following ionic equation:
$$
\mathrm{Pb}(s)+\mathrm{Zn}^{2+}(a q) \longrightarrow \mathrm{Zn}(s)+\mathrm{Pb}^{2+}(a q)
$$
The half-reactions are separated into two compartments. A $\mathrm{Pb}$ electrode is placed in $1.00 \mathrm{M} \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2},$ and a $\mathrm{Zn}$ elec trode in $1.00 \mathrm{M} \mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2} .$ Indicate each of the following for the electrolytic cell:
(a) oxidation half-cell reaction
(b) reduction half-cell reaction
(c) anode and cathode
(d) direction of electron flow
(e) direction of $\mathrm{NO}_{3}^{-}$ in the salt bridge

Sima Sarker

Numerade Educator

Problem 58

The nonspontaneous redox reaction of chromium metal and aqueous aluminum nitrate is an electrolytic process according to the following ionic equation:
$$
\mathrm{Cr}(s)+\mathrm{Al}^{3+}(a q) \longrightarrow \mathrm{Al}(s)+\mathrm{Cr}^{3+}(a q)
$$
The half-reactions are separated into two compartments. A Cr electrode is placed in $1.00 \mathrm{M} \mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3},$ and an $\mathrm{Al}$ electrode in $1.00 \mathrm{M} \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3} .$ Indicate each of the following for the electrolytic cell:
(a) oxidation half-cell reaction
(b) reduction half-cell reaction
(c) anode and cathode
(d) direction of electron flow
(e) direction of $\mathrm{NO}_{3}^{-}$ in the salt bridge

David Collins

Numerade Educator

Problem 59

The nonspontaneous redox reaction of chlorine gas and aqueous sodium fluoride is an electrolytic process according to the following equation:
$$
\mathrm{Cl}_{2}(g)+2 \mathrm{NaF}(a q) \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{F}_{2}(g)
$$
The half-reactions are separated into two compartments. A Pt electrode is placed in $1.00 \mathrm{M} \mathrm{NaCl},$ and a second $\mathrm{Pt}$ electrode in $1.00 \mathrm{M}$ NaF. Indicate each of the following for the electrolytic cell:
(a) oxidation half-cell reaction
(b) reduction half-cell reaction
(c) anode and cathode
(d) direction of electron flow
(e) direction of $\mathrm{Na}^{+}$ in the salt bridge

David Collins

Numerade Educator

Problem 60

The nonspontaneous redox reaction of bromine and aqueous sodium chloride is an electrolytic process according to the following equation:
$$
\mathrm{Br}_{2}(l)+2 \mathrm{NaCl}(a q) \longrightarrow 2 \mathrm{NaBr}(a q)+\mathrm{Cl}_{2}(g)
$$
The half-reactions are separated into two compartments. A Pt electrode is placed in $1.00 \mathrm{M} \mathrm{NaBr}$, and a second $\mathrm{Pt}$ electrode in $1.00 \mathrm{M} \mathrm{NaCl}$. Indicate each of the following for the electrolytic cell:
(a) oxidation half-cell reaction
(b) reduction half-cell reaction
(c) anode and cathode
(d) direction of electron flow
(e) direction of $\mathrm{Na}^{+}$ in the salt bridge

David Collins

Numerade Educator

Problem 61

Calculate the oxidation number for sulfur in calcium thiosulfate, $\mathrm{CaS}_{2} \mathrm{O}_{3}$.

Ivan Kochetkov

Numerade Educator

Problem 62

Calculate the oxidation number for sulfur in sodium tetrathionate, $\mathrm{Na}_{2} \mathrm{~S}_{4} \mathrm{O}_{6}$

Ivan Kochetkov

Numerade Educator

Problem 63

The redox reaction between cobalt metal and aqueous mercury(II) nitrate produces cobalt(II) nitrate and droplets of liquid mercury metal. Write a net ionic equation for the reaction.

Sima Sarker

Numerade Educator

Problem 64

The redox reaction between liquid mercury and aqueous gold(III) acetate produces mercury(I) acetate and gold metal. Write a net ionic equation for the reaction.

David Collins

Numerade Educator

Problem 65

The redox reaction between zinc metal and sulfuric acid produces zinc sulfate and hydrogen gas. Write a net ionic equation for the reaction.

Sima Sarker

Numerade Educator

Problem 66

The redox reaction between aluminum metal and hydrochloric acid produces aluminum chloride and hydrogen gas. Write a net ionic equation for the reaction.

Susan Hallstrom

Susan Hallstrom

Numerade Educator

Problem 67

The redox reaction between lithium metal and water produces lithium hydroxide and hydrogen gas. Write a net ionic equation for the reaction.

Sima Sarker

Numerade Educator

Problem 68

The redox reaction between calcium metal and water produces calcium hydroxide and hydrogen gas. Write a net ionic equation for the reaction.

Sima Sarker

Numerade Educator

Problem 69

Write a balanced equation for the reaction of ethyl alcohol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH},$ and an acidic potassium dichromate solution that occurs in "breathalyzers."
$$
\begin{aligned}
\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(a q)+\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q) & \longrightarrow \\
& \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{Cr}^{3+}(a q)+\mathrm{H}_{2} \mathrm{O}(l)
\end{aligned}
$$

David Collins

Numerade Educator

Problem 70

Write a balanced equation for the reaction of a copper penny in a dilute nitric acid solution.
$$
\mathrm{Cu}(s)+\mathrm{NO}_{3}^{-}(a q) \longrightarrow \mathrm{Cu}^{2+}(a q)+\mathrm{NO}(g)
$$

David Collins

Numerade Educator

Problem 71

Chromium (VI) can cause severe medical problems when ingested. Which organs in the human body are affected and can show symptoms of chromium poisoning?

David Collins

Numerade Educator

Problem 72

Although chromium disposal is an environmental concern, what are some of its current uses?

David Collins

Numerade Educator